A mixture consists of sand and an aqueous saltsolution. Which procedure can be used to separate
the sand, salt, and water from each other?
(1) Evaporate the water, then filter out the salt.
(2) Evaporate the water, then filter out the sand.
(3) Filter out the salt, then evaporate the water.
(4) Filter out the sand, then evaporate the water.

Answers

Answer 1

Answer:

Answer is (4).

Explanation:

The given mixture contains an insoluble solid and an aqueous solution of salt. The insoluble solid is sand.

First we have to separate insoluble solid. Sand can be separated by doing filtration. When we filter the mixture sand can be seen as the residue on the filter paper.

After filtering the mixture, we should collect the filtrate. Filtrate is the salt solution. By doing evaporation we can get the solid salt.

First and second choices are wrong because after evaporating water filtrationcannot be done and salt and sand will be mixed together.

Salt cannot befiltered out because the salt is soluble and it is inaqueous medium. Hence, third choice is wrong

Answer 2

Answer: the best answer is 4 because if you get rid of the sand first and evaporate the water you're left with salt

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How are proteins, carbohydrates, and fats related to the discipline of chemistry?

Answers

can you explain what you're looking for

*food science*
When you consume proteins, carbs, and fats they are chemically changed into energy.

An element's atomic number is the A. weight of the atom.
B. sum of the protons and neutrons in an atom.
C. number of protons in an atom's nucleus.
D. mass of the atom

Answers

Answer:

C. number of protons in an atom's nucleus.

Explanation:

Atomic number : It is defined as the number of electrons or number of protons present in a neutral atom.

However, when we talk about the atomic number of the ion, it is not equal to the number of electrons as electron can be gained or loosed.

This is why, more appropriately, the number of the protons which are present in the nucleus of the atom is called the atomic number.

For example, Sodium has 11 protons in its nucleus which suggest that the atomic number of sodium is 11.

C. the number of protons in nucleus

How are ions Formed?

Answers

Answer & explanation:

For an atom to be electrically neutral, it must have the same amount of protons and electrons, but this does not always happen, so compounds called ions arise.

Ions are formed when an atom of an element has electron gain or loss due to reactions. They can be classified into cations and anions.

Anions are atoms that receive electrons, so they are negatively charged.

Examples: Cl⁻, O⁻², N⁻³

Cations are atoms that lose electrons and thus become positively charged.

Examples: Na⁺, Al⁺³, Pb⁺⁴

In addition, some compounds are formed in bonds between negative and positive ions. These are called ionic bonds.

Example: Formation of sodium chloride (table salt).

Na⁺ + Cl⁻ → NaCl

Ions are formed when atoms lose or gain electrons in order to fulfill the octet rule and have fuller valence electron shells.

Explain why all ores are minerals but all minerals are not ores.

Answers

An ore is a type of rock that contains many minerals. But a mineral is just a part of the ore. So all ores are minerals but all minerals are not ores.

Minerals:Metal bearing substance, found in earth's crust are called minerals
Ore:the Minerals which metals can be obtained on a commercial scale are called Ores
form this definitions we can understand that ores are minerals which is used to obtain metals so, only all ores are minerals but all minerals are not ores.

Gaseous methane (CH₄) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O) If 0.391 g of carbon dioxide is produced from the reaction of 0.16 g of methane and 0.84 g of oxygen gas, calculate the percent yield of carbon dioxide.

Answers

Answer : The percent yield of $CO_2$ is, 68.4 %

Solution : Given,

Mass of $CH_4$ = 0.16 g

Mass of $O_2$ = 0.84 g

Molar mass of $CH_4$ = 16 g/mole

Molar mass of $O_2$ = 32 g/mole

Molar mass of $CO_2$ = 44 g/mole

First we have to calculate the moles of $CH_4$ and $O_2$ .

$\text{ Moles of }CH_4=\frac{\text{ Mass of }CH_4}{\text{ Molar mass of }CH_4}=(0.16g)/(16g/mole)=0.01moles$

$\text{ Moles of }O_2=\frac{\text{ Mass of }O_2}{\text{ Molar mass of }O_2}=(0.84g)/(32g/mole)=0.026moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$CH_4+2O_2\rightarrow CO_2+2H_2O$

From the balanced reaction we conclude that

As, 2 mole of $O_2$ react with 1 mole of $CH_4$

So, 0.026 moles of $O_2$ react with $(0.026)/(2)=0.013$ moles of $CH_4$

From this we conclude that, $CH_4$ is an excess reagent because the given moles are greater than the required moles and $O_2$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $CO_2$

From the reaction, we conclude that

As, 2 mole of $O_2$ react to give 1 mole of $CO_2$

So, 0.026 moles of $O_2$ react to give $(0.026)/(2)=0.013$ moles of $CO_2$

Now we have to calculate the mass of $CO_2$

$\text{ Mass of }CO_2=\text{ Moles of }CO_2* \text{ Molar mass of }CO_2$